(A) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$. For the reaction $2NO_{2(g)} \rightleftharpoons 2N

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(A) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$. For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the change in the number of moles of gaseous products and reactants is $\Delta n = (2 + 1) - 2 = 1$. Substituting $\Delta n = 1$ into the equation,we get $K_p = K_c(RT)^1$. Since $R = 0.083 \ L \cdot bar \cdot K^{-1} \cdot mol^{-1}$ and $T = 184 + 273 = 457 \ K$,the term $(RT) = 0.083 \times 457 \approx 37.93$. Since $(RT) > 1$,it follows that $K_p > K_c$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Easy

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the value of $K_c$ is $1.8 \times 10^{-6}$ at $184^{\circ}C$. Given $R = 0.083 \ L \cdot bar \cdot K^{-1} \cdot mol^{-1}$,compare $K_p$ and $K_c$ at $184^{\circ}C$.

A
$K_p > K_c$
B
$K_p < K_c$
C
$K_p = K_c$
D
$K_p$ depends on the total pressure of the gas.

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$:
$(i)$ $2 NOCl_{(g)} \longleftrightarrow 2 NO_{(g)} + Cl_{2(g)}$; $K_{p} = 1.8 \times 10^{-2}$ at $500 \ K$
$(ii)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$; $K_{p} = 167$ at $1073 \ K$

Medium

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

Medium

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For which of the following reactions does the equilibrium constant depend on the units of concentration?

MediumAIIMS 1983

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For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,the observed total pressure of the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^\circ C$. The value of $K_P$ for the reaction is: (in $atm^2$)

Medium

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For a given exothermic reaction,$K_p$ and $K'_p$ are the equilibrium constants at temperatures $T_1$ and $T_2,$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2,$ where $T_2 > T_1,$ it is readily observed that:

DifficultNEET 2014

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For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the value of $K_c$ is $1.8 \times 10^{-6}$ at $184^{\circ}C$. Given $R = 0.083 \ L \cdot bar \cdot K^{-1} \cdot mol^{-1}$,compare $K_p$ and $K_c$ at $184^{\circ}C$.

Similar Questions

Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$:$(i)$ $2 NOCl_{(g)} \longleftrightarrow 2 NO_{(g)} + Cl_{2(g)}$; $K_{p} = 1.8 \times 10^{-2}$ at $500 \ K$$(ii)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$; $K_{p} = 167$ at $1073 \ K$

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

For which of the following reactions does the equilibrium constant depend on the units of concentration?

For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,the observed total pressure of the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^\circ C$. The value of $K_P$ for the reaction is: (in $atm^2$)

For a given exothermic reaction,$K_p$ and $K'_p$ are the equilibrium constants at temperatures $T_1$ and $T_2,$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2,$ where $T_2 > T_1,$ it is readily observed that:

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Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$:
$(i)$ $2 NOCl_{(g)} \longleftrightarrow 2 NO_{(g)} + Cl_{2(g)}$; $K_{p} = 1.8 \times 10^{-2}$ at $500 \ K$
$(ii)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$; $K_{p} = 167$ at $1073 \ K$